Samantha
Lau
,
Cei B.
Provis-Evans
,
Alexander P.
James
and
Ruth L.
Webster
*
Department of Chemistry, University of Bath, Claverton Down, Bath BA2 7AY, UK. E-mail: r.l.webster@bath.ac.uk
First published on 20th July 2021
The hydroboration of aldehydes, ketones and CO2 is demonstrated using a cheap and air stable [Fe(salen)]2-μ-oxo pre-catalyst with pinacolborane (HBpin) as the reductant under mild conditions. This catalyst system chemoselectively hydroborates aldehydes over ketones and ketones over alkenes. In addition, the [Fe(salen)2]-μ-oxo pre-catalyst shows good efficacy at reducing “wet” CO2 with HBpin at room temperature.
Relative to noble metals, there are significantly fewer reports on using iron complexes to mediate hydroboration of aldehydes and ketones.18–24 Notably in 2017, Findlater and co-workers reported the simple use of a Fe(acac)3/NaHBEt3 system to hydroborate a range of aldehydes and ketones in moderate to excellent yields in the presence of 10 mol% catalyst.25 Following on, Baker, Hein and co-workers demonstrated the use of a [Fe(N2S2)]2 complex at 0.1 mol% catalyst loading to hydroborate aldehydes selectively with TON ca. 5200 easily achieved in one instance.26 In addition, the first case of an iron(II) coordination polymer and heterogeneous Fe2O3 nanoparticles mediated hydroboration of these carbonyl moieties have been reported by Zhang and co-workers27,28 and Geetharani, Bose and co-workers29 respectively. A more difficult but highly desired transformation is the asymmetric hydroboration of ketones to achieve optically active secondary alcohols,1 with only a handful of examples using iron complexes reported to date.23,30
Beyond HB of carbonyl functionality of simple molecules, there has been a paucity in reports of HB of CO2 mediated by iron complexes.31 In 2015, Sabo-Etienne, Bontemps and co-workers32 reported high conversion and selectivity for the formation of bis(boryl)acetal using 9-borabicyclo[3.3.1]-nonane (9-BBN) as the borane source and [Fe(H)2(dmpe)2] (dmpe = 1,2-bis(dimethylphosphino)ethane) as the catalyst.
Continuing from our previous studies using a simple iron salen complex (1a) to effect the hydrophosphination of alkenes33,34 and the cyclotrimerization of alkynes,35 here we report the hydroboration of both aldehydes and ketones with good chemoselectivity observed for aldehydes over ketones. Furthermore, we disclose modest rate of reduction of CO2 with HBpin (Scheme 1).
Excellent yields are achieved across all the aldehydes tested with almost full conversion to the organoborate product observed spectroscopically. Electronic effects para to the benzaldehyde do not influence yields and the system is proficient for both aryl and alkyl aldehydes. 4-Hydroxybenzaldehyde requires a second equivalent of HBpin due to competing reactivity of the hydroxyl group with the reducing reagent (2f). Chemoselectivity is demonstrated with the alkene functionality left intact for cinnamaldehyde and only the mono hydroboration product observed (2h) by NMR spectroscopy. The organoborate products can be converted to their primary alcohol by quenching the reaction with minimal MeOH and then removal of the iron through a silica plug with methylene chloride as the eluent.
The homogeneity of the HB of aldehydes was tested. Complementary results from parallel PMe3 and Hg dropping test suggest the reaction is homogenous in nature (see ESI†).
Hydroboration of ketones requires a higher temperature and longer reaction time. Standard substrate, acetophenone, gives 3a in good spectroscopic yield on 0.25 mmol scale and 58% (0.59 g) isolated yield of 1-phenyl ethan-1-ol when the reaction is scaled by over 30 times (to 8.3 mmol). Good yields are obtained with electron withdrawing groups (3d–f) in the para position with lower conversions found for electron donating groups (3b, 3g) in the same position. The conversions of the ketones are comparable to the recent literature on iron mediated HB of ketones (vide supra). Aliphatic products 3i and 3j are formed in excellent spectroscopic yield. Competitive alkene HB is not observed, for example 3k is produced in low spectroscopic yield but the alkene is unreacted, while we attribute the modest yield of 3m to the volatility of the starting material. Unfortunately, our catalyst system is unable to hydroborate esters or tertiary amides, with less than 5% conversion of starting material observed for the ester substrates; ethyl benzoate, vinyl benzoate, methyl 2-bromobenzoate, methyl formate, and the amide substrates; N,N-diisopropylbenzamide, N-(tert-butyl)-N-isopropyl-3,5-bis(trifluoromethyl)benzamide and, N-(tert-butyl)-N-ethyl-4-methylbenzamide respectively, even at 80 °C with higher equivalents of HBpin used (Fig. 2).
The chemoselectivity of the catalyst system was further investigated; intermolecular competition reactions show the catalytic system selectively hydroborates aldehydes over ketones and ketones over alkenes (Scheme 2a–c). Due to the high conversions across all benzaldehyde derivatives with different electronic properties in the para position, a qualitative intermolecular competition reaction using 4-bromobenzaldehyde, benzaldehyde and 4-methoxybenzaldehyde was set up (Scheme 2d). The calculated spectroscopic conversions show faster reaction with electron withdrawing substituent –Br at the para position relative to electron donating substituent –OMe.
To further interrogate the limits of this catalytic system, the HB of acetophenone derivatives using the chiral iron salen complex 1b under the same reaction conditions was carried out to probe if enantioinduction36 can be conferred to the product (Fig. 3, top). The reactions of the substrates are visibly faster; good to excellent conversions are achieved within 2 h at 60 °C compared to 24 h using 1a. Unfortunately, no enantioinduction is observed in the organoborate products after work-up to the secondary alcohols and reacting these with the chiral auxiliary (R)-Mosher's acid37 to form the corresponding diastereoisomeric ester product.38
The different reactivity observed between 1a and 1b on the HB of ketones may allude to the mechanism involved in these reactions. The varying modes of activation that 1a can undergo have been investigated previously by our group showing potential to form a twisted Fe salen complex containing ‘Bpin’ fragment, or alternatively can simply be reduced down to 1c, an Fe(II) air and moisture sensitive analogue of 1a.34,35 Reacting benzaldehyde with 2 mol% 1c, results in 92% conversion to 2a at room temperature after 2 h which is comparable to the efficacy of 1a (Fig. 3, bottom). This data would suggest the mechanism of the HB of carbonyls is likely to undergo a reduction with HBpin to generate the active species 1c that participates in the catalytic cycle. The empirical observation that 1b is a more active pre-catalyst than 1a could be due to the greater electron density on the iron centre from the tert-butyl groups on the phenolate arms as well as the cyclohexyl backbone of the ligand for a faster reduction to the active Fe(II) species. Further detailed study is necessary to determine whether 1c undergoes further activation (i.e. twisting) to generate an on-cycle species, or whether 1c is a discrete on-cycle catalyst in its own right.
We next examined the reduction of CO2 using 1a as the pre-catalyst.‡ The advantage of using boranes for CO2 reduction circumvents harsher reaction conditions normally associated when using dihydrogen gas as the reductant by exploiting the more reactive B–H bond.39–43 Due to the insolubility of bis (pinacolato)diborane (BOB) formed during the reaction in CD3CN, a 1:1 mixture of CD3CN:C6D6 is used for the following studies. Furthermore, “wet” CO2 generated from dry ice/toluene mixture, and without passing through a drying column, is added directly to the reaction vessel. Modest consumption of HBpin is achieved after 7 days at room temperature, with formation of the formoxy (4), acetal (5), methoxy (6) derivatives of HBpin, and undesired BOB confirmed by 1H and 11B NMR spectroscopy.44 Repeating the reaction at 60 °C shows similar conversions to 4, 5, and 6 but with a higher yield of BOB (see ESI†). Although the rate of the reaction is slow and conversions modest, the use of “wet” CO2 demonstrates the air and moisture stability of 1a in this catalytic transformation and the accessibility of this chemistry without the need of specialist equipment. Reaction with “dry” CO2 from gas cylinder shows similar reactivity and confirmed no detrimental effect in using “wet” CO2.
Alternative borane sources 9-BBN and HBcat were also tested but perform poorly in the reaction; differing from trends observed in the reported literature.31,32,45 Furthermore, no advantageous improvement to reduction of CO2 is observed using 1b as the pre-catalyst. However, the potential to optimise the ligand design of these [Fe(salen)]2-μ-oxo complexes provides an attractive opportunity to improve the rate of CO2 reduction but is beyond the scope of this study (Table 1).
[Fe] | Borane | 4 | 5 | 6 | COa + H2 + R2BOBR2 |
---|---|---|---|---|---|
a 13CO2 reaction performed to try and detect free 13CO or Fe–13CO species. However, these were not observed, potentially due to the small scale of the reaction and paramagnetic nature of any Fe–CO complex formed. | |||||
1a (1 mol%) | HBpin | 5% | 1% | 1% | 8% |
1a (1 mol%) | HBcat | — | — | 12% | 44% |
1a (1 mol%) | 9-BBN | 6% | — | — | — |
1b (1 mol%) | HBpin | — | — | — | 20% |
1c (2 mol%) | HBpin | 8% | 2% | 7% | 22% |
Footnotes |
† Electronic supplementary information (ESI) available: Synthetic methods, analysis data and NMR spectra. See DOI: 10.1039/d1dt02092g |
‡ CO2 reactions performed in a standard J. Young NMR tube. Estimated theoretical maximum amount of CO2 in reaction vessel at 1 atm and 25 °C was calculated to be 0.08 mmol. |
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